Electronic configuration and Molecular Behavior:
- The distribution of electrons among various molecular orbitals is called the electronic configuration of the molecule.
Important information of configuration:
a) Stability of Molecules:
- The molecule is stable if NB is greater than NA
- The molecule is unstable if NB is less than NA.
Where
NB → Bonding e⁻s
NA → Anti – Bonding e⁻s
b) Bond order:
Bond order is defined as one half the difference between the number of electrons present in the bonding and the anti-bonding orbitals.
Bond order = ½ [NB – NA]
The rules discussed in the above regarding the stability of the molecule can be restated in terms of Bond order as follows.
- A positive Bond order means a stable molecule while negative (or) zero bond order means an unstable molecule.
- Nature of Bond: Integral bond order values of 1, 2 (or) 3 correspond to single, double (or) triple bonds respectively.
c) Bond Length:
- The bond order between two atoms in a molecule may be taken as an approximate measure of the Bond length.
- Bond length decreases bond order increases.
d) Magnetic Nature:
- If all the molecular orbitals in a molecule are doubly occupied the substance is diagrammatic.
- If one (or) more molecular orbitals are singly occupied it is paramagnetic.
EX: O₂ Molecule
Bonding in some Homonuclear diatomic molecules:
1. Hydrogen Molecule (H₂):
- There are 2 electrons in hydrogen molecule which are present in σ1S molecular orbital so electronic configuration of hydrogen molecule is H2 : (σ1S)2
The bond order of H₂ molecule can be calculated as given below
Bond order \(=\frac{{{N}_{B}}-{{N}_{a}}}{2}=\frac{2-2}{2}=1\)
- Since there is no unpaired electron in hydrogen molecule, therefore it is diamagnetic.
2. Helium molecule (He₂):
- In He₂ molecule there are 4 electrons. These electrons will be accommodated in σ1S and σ*1S molecular orbital leading to electronic configuration.
He₂ : (σ1S)² (σ*1S)² - Bond order He₂ is ½ (2 – 2) = 0
- He₂ Molecule is therefore unstable and does not exist.
3. Lithium Molecule (Li₂):
- The electronic configuration of lithium is 1S², 2S¹. There are six electrons in Li₂ the electron configuration of Li₂ molecule therefore is Li₂ : (σ1S)² (σ*1S)² (σ2S)²
- The above configuration is also written as KK (σ2S)² where KK represents the closed K shell structure (σ1S)² (σ*1S)²
- There are four electrons present in bonding molecular orbitals and two electrons in anti-bonding molecular orbitals.
Bond order ½ [4 – 1] = 1 - It has no unpaired electrons so it is diamagnetic.
4. Oxygen molecule (O₂):
- The electronic configuration of oxygen atom is 1S²2S²2P⁴ each oxygen atom has 8 electrons hence, in O₂ molecule there are 16 electrons. The electronic configuration of O₂ molecule therefore O₂ : (σ1S)² (σ*1S)² (σ2S)² (σ*2S)² (σ2PZ)² (π2P²X ≡ π2P²Y) (π*2P¹X ≡ π*2P¹Y)
- From the electronic configuration of O₂ molecule, t is clear that ten electrons are present in anti-bonding molecular orbitals and six electrons are present in anti-bonding molecular orbitals.
Its bond order = ½ [NB – NA] = ½ [10 – 6] = 4. - It may be noted that it contains two unpaired electrons π*2PX and π*2PY molecular orbitals.
- O₂ Molecule should be paramagnetic.
5. Nitrogen molecule (N₂):
- The electronic configuration of Nitrogen is 1s² 2S² 2P³, there are 14 electrons in N₂. The electronic configuration of N₂ : σ1S² < σ*1S² < σ2S² < σ*2S² < (π2P²x = π2P²y) < σ2P²z)
- Bond order of N₂ = ½ [10 – 4] = 3
- There is no unpaired electron in the electronic configuration of N₂.
It is diamagnetic in nature.